Chapter 9.4, Problem 9.26QAP

Interpretation Introduction

(a)

Interpretation:

To calculate the amount of Li₂O produced when given amounts of reactants react according to following reaction:

  $\text{4Li(s)}\text{+}{\text{O}}_{\text{2}}\text{(g)}\stackrel{}{\to }{\text{2Li}}_{\text{2}}\text{O}\text{(s)}$

Concept Introduction:

A stoichiometric coefficient of a well-balanced chemical equation tells about the relative relation between moles of reactants used and moles of products formed.

Lets say we have a chemical reaction as:

  $\text{aA}\text{+bB}\to \text{cC}\text{+}\text{dD}$

If above reaction is well-balanced then,

a moles of A reacts with b moles of B to produce c moles of C and d moles of D.

Limiting reactant: It is reactant in a chemical reaction which limits the amounts of products formed.

After complete utilization of limiting reactant, no more products are formed.

Way to determine limiting reactant:

• Calculate moles of each reactant.
• Divide moles of each reactant with their respective stoichiometric coefficient from well-balanced chemical equation.
• Lower value corresponds to the limiting reactant.

Interpretation Introduction

(b)

Interpretation:

To calculate the amount of Fe produced when given amounts of reactants reacts according to following reaction:

  ${\text{Fe}}_{\text{2}}{\text{O}}_{\text{3}}\text{(s)}\text{+}{\text{3H}}_{\text{2}}\text{(g)}\stackrel{}{\to }\text{2Fe}\text{(s)}\text{+}{\text{3H}}_{\text{2}}\text{O}\text{(l)}$

Concept Introduction:

A stoichiometric coefficient of a well-balanced chemical equation tells about the relative relation between moles of reactants used and moles of products formed.

Lets say we have a chemical reaction as:

  $\text{aA}\text{+bB}\to \text{cC}\text{+}\text{dD}$

If above reaction is well-balanced then,

a moles of A reacts with b moles of B to produce c moles of C and d moles of D.

Limiting reactant: It is reactant in a chemical reaction which limits the amounts of products formed.

After complete utilization of limiting reactant, no more products are formed.

Way to determine limiting reactant:

• Calculate moles of each reactant.
• Divide moles of each reactant with their respective stoichiometric coefficient from well-balanced chemical equation.
• Lower value corresponds to the limiting reactant.

Interpretation Introduction

(c)

Interpretation:

To calculate the amount of H₂S produced when given amounts of reactants react according to following reaction:

  ${\text{Al}}_{\text{2}}{\text{S}}_{\text{3}}\text{(s)}\text{+}{\text{6H}}_{\text{2}}\text{O}\text{(l)}\stackrel{}{\to }{\text{2Al(OH)}}_{\text{3}}\text{(aq)}\text{+}{\text{3H}}_{\text{2}}\text{S}\text{(g)}$

Concept Introduction:

A stoichiometric coefficient of a well-balanced chemical equation tells about the relative relation between moles of reactants used and moles of products formed.

Lets say we have a chemical reaction as:

  $\text{aA}\text{+bB}\to \text{cC}\text{+}\text{dD}$

If above reaction is well-balanced then,

a moles of A reacts with b moles of B to produce c moles of C and d moles of D.

Limiting reactant: It is reactant in a chemical reaction which limits the amounts of products formed.

After complete utilization of limiting reactant, no more products are formed.

Way to determine limiting reactant:

• Calculate moles of each reactant.
• Divide moles of each reactant with their respective stoichiometric coefficient from well-balanced chemical equation.
• Lower value corresponds to the limiting reactant.